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BIO 1210 > Chemistry > Flashcards

Chemistry Flashcards

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1
Q

Define matter

A

Anything that takes up space and has mass

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2
Q

Define atom

A

The smallest unit of matter that retains the property of the element and can be broken into 3 subatomic particles (neutron, proton, electron)

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3
Q

T or F: an uncharged atom has a neutral charge

A

True because the electron and proton cancel each other out

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4
Q

What are the 3 subatomic particles that make up an atom?

A
  1. electron
  2. neutron
  3. proton
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5
Q

Define potential energy

A

the energy that matter has because of its location or structure

ex. objects at the top of a hill have more potential energy than those at the bottom

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6
Q

define an electron shell

A

electrons have different energy levels and each shell is representative of an electron’s state of potential energy

the further away an electron is from the nucleus, the higher energy it has

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7
Q

Define compound

A

A substance consisting of 2+ elements in a fixed ratio

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8
Q

Define atomic number

A

Each atom has a unique number that identifies how many protons it has

ex. hydrogen has one proton so it has atomic number 1

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9
Q

Define atomic mass

A

the approximate weight of an atom measured by taking the sum of protons and neutrons

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10
Q

How is the behaviour of an atom determined?

A

By the distribution of electrons in their electron shells

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11
Q

Define valence electrons

A

the electrons in the outermost shell (valence shell)

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12
Q

Define metals and give an example

A

Elements with high electrical conductivity, lustre (shine), and malleability

Readily lose electrons to form positive ions (cations)

ex. H, Li, Mg, Ca, Mn, etc.

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13
Q

Define non-metals and give an example

A

elements that are poor electrical conductors, lack lustre, are brittle and tend to gain electrons to form negative ions (anions)

ex. B, C, N, O, F, etc.

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14
Q

Define electron orbital

A

A 3D space where an electron is found 90% of the time

Each shell consist of a specific number of orbitals

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15
Q

Define chemical bonds

A

an interaction between two atoms

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16
Q

Define covalent bonds

A

An interaction between two atoms in which they share electrons in their valence shells (ie electrons orbit around both atoms)

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17
Q

Define molecule

A

Two or more atoms held together by covalent bonds

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18
Q

Define electronegativity

A

An atom’s strength of attraction for electrons

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19
Q

If an atom is more electronegative, it will have more or less ability to pull electrons from less electronegative atoms?

A

MORE

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20
Q

Define polar covalent bonds

A

Interactions between two atoms in which they are NOT sharing electrons equally. Resulting in partial charges for atoms or molecules

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21
Q

Give an example of a polar covalent bond

A

N-H
O-H
O-C

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22
Q

Define non-polar covalent bonds

A

Interactions between two atoms in which they share electrons because they have the same/similar electronegativity

ex. C-H

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23
Q

Define ionic bonds

A

A weak interaction between two atoms with a large difference in electronegativity so they do not equally share electrons and one atom will strip an electron from the other to form ions.

usually between a metal and non-metal

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24
Q

T or F: ionic bonds are always strong

A

FALSE.

Ionic bonds are weak in water due to the partial charges of water but are very strong in dry environments

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25
Q

Define hydrogen bonds

A

When a hydrogen atom that is covalently bonded to one atom is also attracted to another slightly negative atom of a different molecule

Usually with oxygen or nitrogen

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26
Q

What kind of bond occurs between hydrogens and oxygen in water molecules?

A

two hydrogen atoms are covalently bonded to oxygen to form a POLAR covalent bond

27
Q

Define cohesion

A

when atoms or molecules are attracted to themselves (related to surface tension)

28
Q

Define adhesion

A

When atoms or molecules are attracted to other molecules

29
Q

Define solvent

A

the dissolving agent of a solution

30
Q

Define solution

A

a liquid that is a HOMOGENOUS mixture of substances

31
Q

Define solute

A

A substance that is dissolved in the solution

32
Q

What properties make water so versatile?

A

Hydrogen bonding ability and polarity

33
Q

Define hydrophobic

A

Ionic and non-polar substances that are excluded from water (do not bond with water, ie do not dissolve in water)

34
Q

Define hydrophilic

A

Partially charged or polar substances that can bond with water and dissolve in water

35
Q

Define amphipathic

A

Substances that contain both hydrophobic and hydrophilic regions

ex. phospholipids

36
Q

What pH range does an acid have?

A

< 7

37
Q

What pH range does an base have?

A

> 7

38
Q

What pH is neutral?

A

7

39
Q

Define pH

A

the negative log of the concentration of H+ (in the form of the hydronium ion, H3O+)

40
Q

Define organic chemistry

A

the study of compounds that contain carbon and other elements found in living things

41
Q

Which 4 elements make up about 96% of living things?

A

carbon
hydrogen
oxygen
nitrogen

42
Q

What makes carbon so unique?

A

It has 4 valence electrons and can make 4 covalent bonds

43
Q

Define macromolecules

A

Large molecules composed of carbon-based compounds

44
Q

What are the 4 macromolecules?

A

carbohydrates
lipids
proteins
nucleic acids

45
Q

What are the other 7 elements that are important for life?

A 
Calcium
Phosphorous
Potassium
Sulphur
Sodium
Chlorine
Magnesium
Ca
Cl
K
Mg
Na
P
S
46
Q

Define isomers

A

compounds with the same molecule formula but different structures and properties

47
Q

what are the 3 different kinds of isomers?

A

structural
cis-trans
enantiomers

48
Q

Define structural isomers

A

Compounds with different arrangements of covalent bonds

49
Q

Define cis-trans isomers

A

Compounds with the same covalent bonds but in different spatial arrangements

Cis: the elements are on the same side of the double bond
Trans: the elements are on the opposite side of the double bonds

50
Q

Define enantiomers

A

Compound isomers that are mirror images of each other because they are different in arrangement around the same side of the double bond

51
Q

What are the 9 functional groups to know for this course?

A
  1. hydroxyl
  2. carbonyl
  3. carboxyl
  4. amino
  5. sulfhydryl
  6. phosphate
  7. ester
  8. methyl
  9. aromatic ring
52
Q

Which of the 9 functional groups are hydrophilic?

A 
hydroxyl
carbonyl
carboxyl
amino
sulfhydryl
phosphate
ester
53
Q

What compounds are hydroxyl groups found in?

A

alcohols

54
Q

what are the 2 kinds of carbonyls?

A

ketone: if the carbon is inside the carbon chain
aldehyde: if the carbon is a the end of the carbon chain

55
Q

What is the chemical symbols for hydroxyl group?

A

OH

56
Q

What is the chemical symbols for carbonyl groups?

A

C=O

57
Q

What is the chemical symbols for carboxyl groups?

What function do they provide?

A

-COOH

Act as an acid by donating H+ proton

58
Q

What is the chemical symbols for amino groups?

What function do they provide?

A

NH2

Act as a base by accepting H+ protons

59
Q

What is the chemical symbols for sulfhydryl groups?

What function do they provide?

A

SH

Found in thiols

Stabilize protein structures

60
Q

What is the chemical symbols for phosphate groups?

What function do they provide?

A

-PO3^2-

react with water to release energy

61
Q

What is the chemical symbols for ester groups?

What function do they provide?

A

-COO-

occurs in most natural fats, oils, and DNA

62
Q

What is the chemical symbols for methyl groups?

What function do they provide?

A

CH3

Affects expression of genes and function of hormones

hydrophobic

63
Q

Where are aromatic rings found? Are they hydrophobic or -philic?

A

in amino rings

hydrophobic

64
Q

Define chemical reactions

A

The making or breaking of chemical bonds

BIO 1210 (16 decks)

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